Why might a metallic compound be mistaken for an ionic compound, based on its physical properties?

A. Both metallic and ionic compounds form brittle crystal lattice structures. Thus, they are unable to absorb energy and cannot form new shapes.

B. Both metallic and ionic compounds are composed of metal atoms in a bond. However, only ionic compounds show extreme luster.

C. Both metallic and ionic compounds form ductile compounds. Thus, they are able to be reshaped without breaking the bond of the compound.

D. Both metallic and ionic compounds can conduct electricity when molten. However, only metallic compounds can conduct electricity in a solid state.

Question

01-12-2020
Chemistry

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Why might a metallic compound be mistaken for an ionic compound, based on its physical properties?

A. Both metallic and ionic compounds form brittle crystal lattice structures. Thus, they are unable to absorb energy and cannot form new shapes.

B. Both metallic and ionic compounds are composed of metal atoms in a bond. However, only ionic compounds show extreme luster.

C. Both metallic and ionic compounds form ductile compounds. Thus, they are able to be reshaped without breaking the bond of the compound.

D. Both metallic and ionic compounds can conduct electricity when molten. However, only metallic compounds can conduct electricity in a solid state.

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ibiscollingwood ibiscollingwood · Answer 1 · 2020-12-05T17:03:03+01:00

Answer:

(D). Both metallic and ionic compounds can conduct electricity when molten. However, only metallic compounds can conduct electricity in a solid state.

Explanation:

Metallic compound have the ability to conduct electricity. Since they are Metals they have loosely held electrons which can contribute to electricity conduction.

Ionic compound are brittle physically, ionic compound cannot conduct electricity while being in solid state as the ions are held strongly by electrostatic force of attraction, they can only conduct electricity while they are in molten or aqueous state. In molten state they are forming ions, and ions are free to move within the solution and therefore contribute to electricity conduction.